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Sidana [21]
3 years ago
9

The specific heat of nickel is 0.44 J/g*⁰C. How much energy needed to change the temperature of 95.4g of nickel from 22⁰C to 32⁰

C. Is the energy absorbed or released?
Chemistry
2 answers:
valentinak56 [21]3 years ago
8 0
To determine the heat or energy needed for the process, we use the equation,
                                               H  = mcpdT
where m is the mass, cp is the specific heat and dT is the temperature difference. 
                                               H = (95.4g)(0.44 J/g°C)(32°C - 22°C)
                                                   = 419.76 J
Thus, the amount of heat that should be ABSORBED is approximately 419.76 J. 
labwork [276]3 years ago
8 0

Answer : The amount of energy needed is, 419.76 J and the energy is absorbed.

Solution :

Formula used :

Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})

where,

Q = heat gained or absorbed = ?

m = mass of nickel = 95.4 g

c = specific heat of nickel = 0.44J/g^oC      

\Delta T=\text{Change in temperature}  

T_{final} = final temperature = 32^oC

T_{initial} = initial temperature = 22^oC

Now put all the given values in the above formula, we get

Q=95.4g\times 0.44J/g^oC\times (32-22)^oC

Q=419.76J

The value of Q is positive that means energy is absorbed.

Therefore, the amount of energy needed is, 419.76 J and the energy is absorbed.

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